Respuesta :
The volume of the titrant, or in our example, the volume of the strong base, is graphed against the pH to create the titration curve. The titration curves of weak acids with strong bases have a number of properties.
The initial pH is more or less acidic than the titration of a strong acid (before the addition of any strong base).
At the start of the titration, the pH increases significantly. This occurs as a result of the weak acid's anion changing into a common ion, which lessens the acid's ability to ionize. Following the initial, abrupt increase, the titration curve only modifies gradually. This is a result of the solution's role as a buffer.
This will carry on until the base exceeds the capacity of the buffers. Half-neutralization takes place at the center of this progressively sloping curve. The concentration of the weak acid and the concentration of its conjugate base are now equal. As a result, pH=pKa. Because only half of the acid has been neutralized, this moment is known as the half-neutralization.
Since all of the acid (HA) has been changed to its conjugate base (A-) by the injection of NaOH, the pH is greater than 7 at this time. As the equilibrium shifts back towards HA, hydroxide is produced, which is represented by the formula: A+H2OAH+OH (2)Prior to the equivalence point, the curve has a brief steep section. It typically doesn't start until a pH of about 10.
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